Embibe Experts Solutions for Chapter: Chemical Kinetics, Exercise 4: Exercise 4

According to the adsorption theory of catalysis, the speed of the reaction increases because:

The two-third life $\left({\mathrm{t}}_{2/3}\right)$ of a first order reaction in which $\mathrm{k}=5.48\times {10}^{-14} \mathrm{per} \sec ,$ is 

For the reaction, 

$2\mathrm{A} +\mathrm{B}\stackrel{}{\to }3\mathrm{C} + \mathrm{D},$

which of the following does NOT express the reaction rate?

The rate of a first-order reaction is $0.04 \mathrm{mol} {\mathrm{l}}^{-1} {\mathrm{s}}^{-1}$ at $10$ seconds and $0.03 \mathrm{mol}{}^{-1} {\mathrm{s}}^{-1}$ at $20$ seconds after initiation of the reaction. The half-life period of the reaction is:

The rate of a chemical reaction doubles for every $10 º\mathrm{C}$ rise of temperature. If the temperature is raised by $50 º\mathrm{C}$, the rate of the reaction increases by about.

Higher order ($>3$) reactions are rare due to _______.

Two reactions ${\mathrm{R}}_{\mathrm{1}} \text{and} {\mathrm{R}}_{\mathrm{2}}$ have identical pre-exponential factors. Activation energy of ${\mathrm{R}}_{\mathrm{1}}$ exceeds that of ${\mathrm{R}}_{\mathrm{2}}$ by $10 \mathrm{kJ} {\mathrm{mol}}^{-1}$. If ${\mathrm{k}}_{\mathrm{1}}\text{ and }{\mathrm{k}}_{\mathrm{2}}$ are rate constants for reactions ${\mathrm{R}}_{\mathrm{1}} \text{and} {\mathrm{R}}_{\mathrm{2}}$, respectively at $300 \mathrm{K}$, $\ln \left(\frac{{\mathrm{k}}_2}{{\mathrm{k}}_1}\right)$ is equal to:
$(\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}\mathrm{)}$

For a reaction, consider the plot of In $\mathrm{k}$ versus $1/\mathrm{T}$ given in the figure. If the rate constant of this reaction at $400 \mathrm{K}$ is ${10}^{-5}{ \mathrm{s}}^{-1}$, then the rate constant at $500 \mathrm{K}$ is :